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Elanso [62]
2 years ago
8

What is the pH of 5.0 L of an aqueous solution that contains 1.0 grams of HBr and 1.0 grams of nitric acid

Chemistry
1 answer:
Nady [450]2 years ago
8 0

Hello!:

Molar mass:

HBr = 80.91 g/mol

HNO3 = 63.01 g/mol

Number of moles:

moles HBr =  1.0 / 80.91 => 0.01235 moles of HBr

moles HNO3 = 1.0 / 63.01 => 0.01587 moles of HNO3

So , total moles of H⁺ :

0.01235 + 0.01587 => 0.02822 moles of H⁺

Molarity of solution:

M = n / V

M = 0.02822 / 5.0

M = 0.005644

Therefore:

pH = - log [ H⁺ ]

pH = - log [ 0.005644 ]

pH = 2.25


Hope that helps!


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If molarity and volume is given then, moles of solute is molarity times volume in liters.

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6 0
3 years ago
The lock-and-key model and the induced-fit model are two models of enzyme action explaining both the specificity and the catalyt
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